This quiz works best with JavaScript enabled. Home > Cbse > Class 11 > Science > Chemistry Part I > Class 11 Chemistry (Part I) Chapter 4 Chemical Bonding And Molecular Structure – Quiz 3 🏠 Homepage 📘 Download PDF Books 📕 Premium PDF Books Class 11 Chemistry (Part I) Chapter 4 Chemical Bonding And Molecular Structure Quiz 3 (60 MCQs) Quiz Instructions Select an option to see the correct answer instantly. 1. What happens to the valence electrons in the formation of a covalent bond? A) They are shared. B) They are gained. C) They remain unchanged. D) They are lost. Show Answer Correct Answer: A) They are shared. 2. Which of the following pair is expected to have the same bond order? A) O$_{2}$$^{-}$, N$_{2}$$^{-}$. B) O$_{2}$ $^{-}$, N$_{2}$$^{+}$. C) O$_{2}$$^{+}$, N$_{2}$$^{-}$. D) O$_{2}$, N$_{2}$. Show Answer Correct Answer: C) O$_{2}$$^{+}$, N$_{2}$$^{-}$. 3. Among the following, which has greater dipole moment? A) BF3. B) NF3. C) NH3. D) None of the above. Show Answer Correct Answer: C) NH3. 4. True or False:Everything on Earth (and the universe!) is made of different combinations of the elements found on the Periodic Table. A) False. B) True. C) All the above. D) None of the above. Show Answer Correct Answer: B) True. 5. What is the formal charge of an atom in a Lewis structure? A) Total bonding electrons only. B) Total valence electrons minus bonding electrons. C) Total valence electrons minus both lone and bonding electrons. D) Total valence electrons minus lone pair electrons. Show Answer Correct Answer: C) Total valence electrons minus both lone and bonding electrons. 6. A covalent bond in which the bonded atoms have an unequal attraction A) Electronegativity. B) Nonpolar bond. C) Diatomic. D) Polar bond. Show Answer Correct Answer: D) Polar bond. 7. The number of types of bonds between two carbon atoms in calcium carbide is A) One sigma, two pi. B) One sigma, one pi. C) Two sigma, two pi. D) Two sigma, one pi. Show Answer Correct Answer: A) One sigma, two pi. 8. State the electronic geometry, Bond angle and Molecular shape of SO2 Molecule A) Tetrahedral, 109.5$^\circ$, Trigonal pyramidal. B) Trigonal planar, 120$^\circ$, Trigonal planar. C) Trigonal planar, less than 120$^\circ$, Angular/Bent. D) None of the above. Show Answer Correct Answer: C) Trigonal planar, less than 120$^\circ$, Angular/Bent. 9. Diphosphorus pentoxide A) P$_{2}$O$_{5}$. B) PO$_{5}$. C) P$_{5}$O$_{2}$. D) P$_{2}$O$_{6}$. Show Answer Correct Answer: A) P$_{2}$O$_{5}$. 10. Lewis pictured an atom in terms of a ..... A) Stable Kernel. B) Positively charged Kernel. C) Negatively charged Kernel. D) None of the above. Show Answer Correct Answer: B) Positively charged Kernel. 11. Which of the following statements about molecular orbitals is true? A) They do not follow the Pauli exclusion principle. B) They can only be formed from s orbitals. C) They are always higher in energy than atomic orbitals. D) They are formed by the combination of atomic orbitals. Show Answer Correct Answer: D) They are formed by the combination of atomic orbitals. 12. Which of the following statement is true? (2001E) A) Hybridisation of the central atom in NH3 and CH4 is SP2. B) BeCl2 has "V" shape while SO2 is linear. C) SF6 is octahedral and F-S-F bond angle is 90$^\circ$. D) CO2 has dipole moment. Show Answer Correct Answer: C) SF6 is octahedral and F-S-F bond angle is 90$^\circ$. 13. Which of the following molecular shapes would have a bond angle of 180 Degrees? A) Bent. B) Linear. C) Trigonal Planar. D) Tetrahedral. Show Answer Correct Answer: B) Linear. 14. Which of the following compounds does not follow the octet rule? A) NaCl. B) H2O. C) CH4. D) BCl3. Show Answer Correct Answer: D) BCl3. 15. For which of the follwoing hybridisation the bond angle is maximum? A) Sp. B) Sp2. C) Sp3. D) DSp2. Show Answer Correct Answer: A) Sp. 16. In the Lewis structure of CO, how many total valence electrons are used? A) 12. B) 6. C) 10. D) 8. Show Answer Correct Answer: C) 10. 17. A nonpolar covalent bond is unlikely when two atoms of different elements join because the atoms are likely to differ in A) Polarity. B) Density. C) Electronegativity. D) State of matter. Show Answer Correct Answer: C) Electronegativity. 18. Chemical bonds form when atoms A) Share or transfer electrons. B) Gain protons. C) Combined nuclei. D) Give up neutrons. Show Answer Correct Answer: A) Share or transfer electrons. 19. What happens to the bond length as bond order increases? A) Bond length becomes unpredictable. B) Bond length decreases. C) Bond length increases. D) Bond length remains the same. Show Answer Correct Answer: B) Bond length decreases. 20. What are non-bonding or lone pairs? A) The pairs of electrons not involved in forming the covalent bond. B) The number of electrons involved in forming the covalent bond. C) The number of electrons not involved in forming the covalent bond. D) The pairs of electrons involved in forming the covalent bond. Show Answer Correct Answer: A) The pairs of electrons not involved in forming the covalent bond. 21. Which of the following has least bond energy? (2000 M) A) H2. B) F2. C) O2. D) N2. Show Answer Correct Answer: B) F2. 22. What is the shape of a molecule with the formula AB3E2? A) Trigonal planar. B) T-shaped. C) Linear. D) Bent. Show Answer Correct Answer: B) T-shaped. 23. True or False:All elements can bond to form molecules. A) True. B) False. C) All the above. D) None of the above. Show Answer Correct Answer: B) False. 24. A Bond formed by mutual sharing of electrons is called as A) Ionic bond. B) Covalent Bond. C) Hydrogen bond. D) None of the above. Show Answer Correct Answer: B) Covalent Bond. 25. When 2 lone pairs and 2 bond pair are around the central atom, reduction in the bond angle is up to- A) B. 104.5$^\circ$. B) 107.5$^\circ$. C) 109.5$^\circ$. D) 102$^\circ$. Show Answer Correct Answer: A) B. 104.5$^\circ$. 26. The pairs of valence electrons that are not shared A) Central atom. B) Lone pair. C) Terminal atom. D) Bonded pair. Show Answer Correct Answer: B) Lone pair. 27. What is the hybridization of the central atom in BCl3? A) Sp. B) Sp2. C) Sp3. D) Dsp3. Show Answer Correct Answer: B) Sp2. 28. The bond angle for a trigonal planar molecule is A) 90 Degrees. B) 180 Degrees. C) 109.5 Degrees. D) 120 Degrees. Show Answer Correct Answer: D) 120 Degrees. 29. Lewis postulated that atoms the noble octet when they are linked by ..... A) Ionic bonds. B) Covalent bonds. C) Chemical bonds. D) None of the above. Show Answer Correct Answer: C) Chemical bonds. 30. According to VSEPR theory, what is the shape of SF$_{4}$? A) Square planar (6 bp, 2 lp). B) Tetrahedral (4 bp, 0 lp). C) See-saw shaped (4 bp, 1 lp). D) Trigonal bipyramidal (5 bp, 0 lp). Show Answer Correct Answer: C) See-saw shaped (4 bp, 1 lp). 31. In the formation of NaCl, what happens to the electron from sodium? A) It remains with sodium. B) It is shared with chlorine. C) It is gained by sodium. D) It is lost to chlorine. Show Answer Correct Answer: D) It is lost to chlorine. 32. What is the concept introduced by G.N. Lewis to represent valence electrons in an atom? A) Rutherford Model. B) Dalton Model. C) Lewis Symbols. D) Bohr Model. Show Answer Correct Answer: C) Lewis Symbols. 33. An element X reacts with chlorine to form a solid of formula XCl. What could be the electronic structure of X? A) 1s$^{2}$ 2s$^{2}$ 2p$^{4}$. B) 1s$^{2}$ 2s$^{2}$ 2p$^{6}$ 3s$^{2}$ 3p$^{5}$. C) 1s$^{2}$ 2s$^{2}$ 2p$^{6}$ 3s$^{1}$. D) 1s$^{2}$ 2s$^{2}$ 2p$^{6}$ 3s$^{2}$. Show Answer Correct Answer: C) 1s$^{2}$ 2s$^{2}$ 2p$^{6}$ 3s$^{1}$. 34. What is the shape of a molecule with the formula AB4E? A) Bent. B) T-shaped. C) See-saw. D) Trigonal pyramidal. Show Answer Correct Answer: C) See-saw. 35. Assertion (A):I3-is linear Reason (R):It is not in sp hybridised state. The correct answer is A) Both A and R are true and R is the correct explanation of A. B) Both A and R are true but R is not the correct explanation of A. C) A is true, R is not true. D) A is not true but R is true. Show Answer Correct Answer: B) Both A and R are true but R is not the correct explanation of A. 36. Which of the following types of hybridisation lead to three dimensional geometry of bonds around carbon atom A) Sp. B) Sp2. C) Sp3. D) None of the above. Show Answer Correct Answer: C) Sp3. 37. What is the bond angle in a water (H2O) molecule? A) 120 degrees. B) 180 degrees. C) 90 degrees. D) 104.5 degrees. Show Answer Correct Answer: D) 104.5 degrees. 38. Geometry having ..... Repulsion b/w electron pair is most suitable electronic geometry. A) Minimum. B) Maximum. C) Neutral. D) None of the above. Show Answer Correct Answer: A) Minimum. 39. What is the result of multiple bonding between two atoms? A) Sharing of two electron pairs. B) Sharing of one electron pair. C) Sharing of four electron pairs. D) Sharing of three electron pairs. Show Answer Correct Answer: A) Sharing of two electron pairs. 40. What is the octet rule primarily based on? A) The chemical inertness of noble gases. B) The temperature of the reaction. C) The chemical reactivity of alkali metals. D) The size of the atoms involved. Show Answer Correct Answer: A) The chemical inertness of noble gases. 41. What type of bond involves the overlap of parallel orbitals? A) Sigma bond. B) Pi bond. C) Ionic bond. D) Metallic bond. Show Answer Correct Answer: B) Pi bond. 42. Which one of the following statements is not correct for sigma and pi bonds between two carbon atoms? A) Sigma bond is stronger than pi bond. B) Bond energies of sigma and pi bonds are of the order of 264 kJ /mol. C) Free rotation of atoms around a sigma bond is allowed but not in case of a pi bond. D) Sigma bond is formed from hybridised orbital and pi bond is formed from unhybridised orbital. Show Answer Correct Answer: B) Bond energies of sigma and pi bonds are of the order of 264 kJ /mol. 43. Which one of the following is the correct set with reference to molecular formula, hybridisation of central atom and shape of the molecule? (2002-M) A) BeCl2, sp, linear. B) H2O, sp, linear. C) H2O, sp, bent. D) CO2, sp, bent. Show Answer Correct Answer: A) BeCl2, sp, linear. 44. In a chemistry class, Ria is learning about the formation of NaCl. She wonders what happens to the electron from sodium during this process. A) It is shared with chlorine. B) It is lost to chlorine. C) It remains with sodium. D) It is gained by sodium. Show Answer Correct Answer: B) It is lost to chlorine. 45. Which of the following has the lowest bond angle? (2000 E) A) NH3. B) H2S. C) CH4. D) H2O. Show Answer Correct Answer: B) H2S. 46. Which of the following molecule is T shaped? A) H2O. B) SF4. C) ClF3. D) NH3. Show Answer Correct Answer: C) ClF3. 47. Why do molecules like hydrogen and oxygen exist as diatomic molecules rather than single atoms? A) Single atoms are unstable and have incomplete electron shells. B) Single atoms are too large to exist independently. C) Single atoms have too many electrons to form bonds. D) Single atoms are more reactive than diatomic molecules. Show Answer Correct Answer: A) Single atoms are unstable and have incomplete electron shells. 48. In VSEPR theory, which type of electron pair has the greatest repulsion? A) Lone pair-bond pair. B) Lone pair-lone pair. C) Bond pair-bond pair. D) Bond pair-lone pair. Show Answer Correct Answer: B) Lone pair-lone pair. 49. What theory explains the formation of chemical bonds based on atomic orbitals, electronic configurations, and overlap criteria? A) VSEPR Theory. B) Molecular Orbital Theory. C) Valence Bond Theory. D) Lewis Theory. Show Answer Correct Answer: C) Valence Bond Theory. 50. The sp$^{3}$d$^{2}$ hybridization of central atom of a molecule would lead to A) Square planar geometr. B) Octahedral geometry. C) Tetrahedral geometry. D) Trigonal bipyramidal geometry. Show Answer Correct Answer: B) Octahedral geometry. 51. In a DNA molecule, which type of bond holds the two strands together? A) Ionic bonds. B) Covalent bonds. C) Hydrogen bonds. D) Metallic bonds. Show Answer Correct Answer: C) Hydrogen bonds. 52. Which of the following statement is wrong for hyrogen bond? A) Hydrogen bond is weaker than covalent bond. B) Hydrogen bond is stronger than vander waals forces of attraction. C) Intermolecular hydrogen bonding is weaker han intramolecular hydrogen bond. D) None of the above. Show Answer Correct Answer: C) Intermolecular hydrogen bonding is weaker han intramolecular hydrogen bond. 53. How does the concept of bond dissociation energy relate to the stability of a molecule? A) Lower bond dissociation energy indicates a more stable molecule. B) Bond dissociation energy does not affect molecular stability. C) Higher bond dissociation energy indicates a more stable molecule. D) Bond dissociation energy is only relevant for ionic bonds. Show Answer Correct Answer: C) Higher bond dissociation energy indicates a more stable molecule. 54. Which one shows high %age of the ionic character? A) HBr. B) HCl. C) H$_{2}$O. D) HF. Show Answer Correct Answer: D) HF. 55. Which one of the following is a planar molecule? (2003-M) A) BCl3. B) NH3. C) HO+. D) PCl3. Show Answer Correct Answer: A) BCl3. 56. Which of the following statement is not correct (2004-M) A) One of the favourable conditions for the formation of cation is low ionisation potential. B) Co-ordination number of Cs in CsCl is 8. C) Ionic bond is directional. D) Ionic compounds have high melting and boiling points. Show Answer Correct Answer: C) Ionic bond is directional. 57. VSEPR is based on the assumption that A) Positive ions attract negative ions. B) Electrons in molecules repel each other. C) Sp$^{2}$ hybridization occurs. D) Positive ions repel each other. Show Answer Correct Answer: B) Electrons in molecules repel each other. 58. Is high melting point a characteristic of most metals? If yes, explain how metallic bonding accounts for this property. A) Yes, because metallic bonds are strong. B) No, because metallic bonds are weak. C) Yes, because metallic bonds are ionic. D) No, because metallic bonds are covalent. Show Answer Correct Answer: A) Yes, because metallic bonds are strong. 59. What does the lattice enthalpy of an ionic solid represent? A) The energy required to completely separate one mole of a solid ionic compound into gaseous ions. B) The energy required to form a gas from a solid. C) The energy required to ionize a neutral atom. D) The energy released during the formation of a solid. Show Answer Correct Answer: A) The energy required to completely separate one mole of a solid ionic compound into gaseous ions. 60. Explain why the bond length is shorter in a stronger bond. Which of the following is the most accurate reasoning? A) Stronger bonds have fewer electrons, reducing the distance. B) Stronger bonds involve greater overlap of orbitals, pulling nuclei closer. C) Stronger bonds involve weaker forces, allowing nuclei to come closer. D) Stronger bonds are formed by larger atoms, reducing the bond length. Show Answer Correct Answer: B) Stronger bonds involve greater overlap of orbitals, pulling nuclei closer. ← PreviousNext →Related QuizzesScience QuizzesClass 11 QuizzesClass 11 Chemistry (Part I) Chapter 4 Chemical Bonding And Molecular Structure Quiz 1Class 11 Chemistry (Part I) Chapter 4 Chemical Bonding And Molecular Structure Quiz 2Class 11 Chemistry (Part I) Chapter 4 Chemical Bonding And Molecular Structure Quiz 4Class 11 Chemistry (Part I) Chapter 4 Chemical Bonding And Molecular Structure Quiz 5Class 11 Chemistry (Part I) Chapter 1 Some Basic Concepts Of Chemistry QuizClass 11 Chemistry (Part I) Chapter 2 Structure Of Atom QuizClass 11 Chemistry (Part I) Chapter 3 Classification Of Elements And Periodicity In Properties QuizClass 11 Chemistry (Part I) Chapter 6 Thermodynamics Quiz 🏠 Back to Homepage 📘 Download PDF Books 📕 Premium PDF Books